**Quantum Numbers**

**Pauli Exclusion Principle: no two electrons can have the**

same set of four quantum numbers

same set of four quantum numbers

1st - Principle QN

n2nd - Orbital QN

l3rd - Magnetic QN

m_{l}4th - Spin QN

m_{s}n = 1,2,3...7 l goes from 0 to n-1

withinan energy levell values = 0 (for s), 1(for p), 2 (for d), 3 (for f) sublevels

Values of m _{l}go from +l to - l , which gives 2l + 1 number of valueshas 2 values:

+1/2 (spin up) and -1/2(spin down)1. measures the average distanceof the e^{-}from the nucleus1. indicates the shape of the orbital ( set of probable locations of the e ^{- })1. identifies the direction the e ^{-}orbital has around the nucleus1. identifies the "spin" or rotationof the e^{-}about its own axis2. different values of nmean different energy levels2. diff. values of lmean diff sublevels. In a sublevel all the e^{-}have nearly the same energy.2. specifies the e ^{-}orbital in which the e^{-}is located within a sublevel.2. shows that each orbitalcan contain only 2 e^{-}3. different values of nmean relatively large differences in the energies of the e^{-}s3. different sublevels

withinthe same level may have moderately large differences in energy.3. different values of m _{l}mean little difference in energies of the e^{-}3. the direction of spin is either in one direction or the other 4. the smallest avgerage distance and the lowest energy occurs when n = 1; each increase in nincreases those quantities.4. within any level, the lowest energy sublevel is s, then p, then d, then f. 4. the number of possible values of m _{l}within a sublevel idenities how many e^{-}pairs that the sublevel can hold4. when 2 e ^{-}(in an atom) have the same set of QN except for m_{s}, then these e^{-}are called an e^{-}pair5. the number of e ^{-}possible in a level is 2n^{2}5. the number of possible values of l for a level is equal to the value of n5.these e ^{-}within an e^{-}pair have essentially the same energy

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